The initial rates of the reaction represented by the equation below were measured in three separate trials at \(298 \text{ K}\).

\[ 2\text{NO}_2(g) + \text{F}_2(g) \rightarrow 2\text{NO}_2\text{F}(g) \]

Trial	\([\text{NO}_2]\ (\text{M})\)	\([\text{F}_2]\ (\text{M})\)	Initial Rate of Formation of \(\text{NO}_2\text{F}\ (\text{M}\cdot\text{s}^{-1})\)
1	\(0.10\)	\(0.10\)	\(2.0 \times 10^{-4}\)
2	\(0.20\)	\(0.10\)	\(4.0 \times 10^{-4}\)
3	\(0.20\)	\(0.30\)	\(1.2 \times 10^{-3}\)

Based on the data in the table, which of the following is the correct rate law and overall reaction order for the reaction?